Chemical Engineering Thermodynamics II
Phase and chemical reaction equilibrium: chemical potential, partial molar properties, fugacity and cubic equations of state, activity coefficient models, azeotropes, flash calculations, liquid-liquid and solid-liquid equilibrium and reaction equilibrium, applied to drying ethanol and a new ethyl acetate line at an ethanol plant in Cedar Rapids, Iowa.
CHE-320 Year 3 3 credits 12 lessons · 4 h 20 min ▶ Video lessons coming soon
Offered by HSM University · Chemical Engineering
This is the American version of this course. See the Canadian version.
What you'll learn
- Use the fundamental property relation and the Gibbs energy to state the criteria of phase and chemical equilibrium, and calculate chemical potentials of ideal-gas mixtures.
- Calculate partial molar, mixing and excess properties of binary solutions, apply the Gibbs-Duhem equation, and explain volume changes on blending ethanol and water.
- Calculate fugacity and fugacity coefficients of pure gases and liquids from the virial and cubic equations of state, including the Poynting correction.
- Apply mixing rules and binary interaction parameters to find fugacity coefficients of species in gas mixtures, and explain the limits of the Lewis-Randall rule.
- Perform bubble point and dew point calculations with Raoult's law and the Antoine equation, and use Henry's law for dissolved gases.
- Calculate activity coefficients and excess Gibbs energies from vapor-liquid data with modified Raoult's law, and test data for thermodynamic consistency.
- Fit and compare the Margules, van Laar, Wilson and NRTL models, and describe the role of UNIFAC in screening mixtures without data.
- Locate binary azeotropes, explain how they move with pressure, and compare entrainer, extractive, pressure-swing and adsorption routes to dry ethanol.
- Solve isothermal flash problems with the Rachford-Rice equation and composition-dependent K-values, and calculate equilibrium water content of compressed gases.
- Calculate liquid-liquid equilibrium, solute distribution and single-stage extraction, and solid-liquid freezing points from activity coefficients.
- Calculate equilibrium constants and equilibrium conversions from standard Gibbs energies, the van 't Hoff equation, pressure, inerts and excess reactants.
- Select and justify thermodynamic property methods for each section of a process, and document the data, checks and uncertainties in a design basis.
Course content
12 lessons · 4 h 20 min total · final exam
- 1 The fundamental property relation and chemical potential 22 min · quiz
- 2 Partial molar properties and mixing 22 min · quiz
- 3 Fugacity of pure fluids and cubic equations of state 21 min · quiz
- 4 Fugacity in mixtures and mixing rules 22 min · quiz
- 5 Raoult's law, bubble points and dew points 21 min · quiz
- 6 Modified Raoult's law and activity coefficients 21 min · quiz
- 7 Activity coefficient models 20 min · quiz
- 8 Azeotropes and strongly non-ideal mixtures 20 min · quiz
- 9 High-pressure equilibrium and flash calculations 23 min · quiz
- 10 Liquid-liquid and solid-liquid equilibrium 22 min · quiz
- 11 Chemical reaction equilibrium 21 min · quiz
- 12 Capstone: choosing a thermodynamic model for the ethyl acetate line 25 min · quiz
- E Final exam 20 questions
Requirements
Recommended background. You can start any course at any time.
Description
Phase and chemical reaction equilibrium: chemical potential, partial molar properties, fugacity and cubic equations of state, activity coefficient models, azeotropes, flash calculations, liquid-liquid and solid-liquid equilibrium and reaction equilibrium, applied to drying ethanol and a new ethyl acetate line at an ethanol plant in Cedar Rapids, Iowa.
Part of the Engineering stream, typically taken in year 3.